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propane a fuel that is used in camp stoves produces carbon dioxide and water vapor on combustion follows given that the molar mass of h2o is 18.02g/mol how many liters of propane are required at sfo to produce 75g of h2o from this reaction

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daniel987
the reaction is : C3H8 + 5O2 ===> 3CO2 + 4H2O

find the number of moles of H2O using the molar mass of H2O 

moles of H2O = 75g/18.02 g/mol = 4.162 moles 

go between the H2O and the propane to find the mole of propane

4.162 moles H2O its a 1 : 4 ratio so divide 4.162 / 4 = 1.041mol of propane

use this equation to find the volume of gas required : V = nRT/P

n is the moles of gas (propane)

R is the universal gas constant (0.082057338)

T is the temperature of the gas (273K)

V = (1.041) x (0.08206 L-atm/mol-K) x (273K)/(1 atm)

V = 23.3 L of C3H8

hope that helps


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